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LECTURE PRESENTATIONS
For CAMPBELL BIOLOGY, NINTH EDITION Jane B. Reece, Lisa A. Urry, Michael L. Cain, Steven A. Wasserman, Peter V. Minorsky, Robert B. Jackson
© 2011 Pearson Education, Inc.
Lectures by
Erin Barley
Kathleen Fitzpatrick
An Introduction to Metabolism
Chapter 8
Overview: The Energy of Life
• The living cell is a miniature chemical factory
where thousands of reactions occur
• The cell extracts energy and applies energy to
perform work
• Some organisms even convert energy to light,
as in bioluminescence
© 2011 Pearson Education, Inc.
Figure 8.1
Concept 8.1: An organism’s metabolism
transforms matter and energy, subject to the
laws of thermodynamics
• Metabolism is the totality of an organism’s
chemical reactions
• Metabolism is an emergent property of life that
arises from interactions between molecules within
the cell
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Organization of the Chemistry of Life into
Metabolic Pathways
• A metabolic pathway begins with a specific
molecule and ends with a product
• Each step is catalyzed by a specific enzyme
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Figure 8.UN01
Enzyme 1 Enzyme 2 Enzyme 3
Reaction 1 Reaction 2 Reaction 3 Product Starting
molecule
A B C D
• Catabolic pathways release energy by
breaking down complex molecules into
simpler compounds
• Cellular respiration, the breakdown of glucose
in the presence of oxygen, is an example of a
pathway of catabolism
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• Anabolic pathways consume energy to build
complex molecules from simpler ones
• The synthesis of protein from amino acids is an
example of anabolism
• Bioenergetics is the study of how organisms
manage their energy resources
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Forms of Energy
• Energy is the capacity to cause change
• Energy exists in various forms, some of which
can perform work
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• Kinetic energy is energy associated with motion
• Heat (thermal energy) is kinetic energy
associated with random movement of atoms or
molecules
• Potential energy is energy that matter possesses
because of its location or structure
• Chemical energy is potential energy available for release in a chemical reaction
• Energy can be converted from one form to another
© 2011 Pearson Education, Inc.
Animation: Energy Concepts
Figure 8.2 A diver has more potential energy on the platform than in the water.
Diving converts potential energy to kinetic energy.
Climbing up converts the kinetic energy of muscle movement to potential energy.
A diver has less potential energy in the water than on the platform.
The Laws of Energy Transformation
• Thermodynamics is the study of energy
transformations
• A isolated system, such as that approximated by
liquid in a thermos, is isolated from its
surroundings
• In an open system, energy and matter can be
transferred between the system and its
surroundings
• Organisms are open systems
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The First Law of Thermodynamics
• According to the first law of thermodynamics,
the energy of the universe is constant
– Energy can be transferred and transformed,
but it cannot be created or destroyed
• The first law is also called the principle of
conservation of energy
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The Second Law of Thermodynamics
• During every energy transfer or transformation,
some energy is unusable, and is often lost as
heat
• According to the second law of thermodynamics
– Every energy transfer or transformation increases the entropy (disorder) of the universe
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Figure 8.3
(a) First law of thermodynamics (b) Second law of thermodynamics
Chemical energy
Heat
Figure 8.3a
(a) First law of thermodynamics
Chemical energy
Figure 8.3b
(b) Second law of thermodynamics
Heat
• Living cells unavoidably convert organized
forms of energy to heat
• Spontaneous processes occur without
energy input; they can happen quickly or
slowly
• For a process to occur without energy input, it
must increase the entropy of the universe
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Biological Order and Disorder
• Cells create ordered structures from less
ordered materials
• Organisms also replace ordered forms of
matter and energy with less ordered forms
• Energy flows into an ecosystem in the form
of light and exits in the form of heat
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Figure 8.4
Figure 8.4a
Figure 8.4b
• The evolution of more complex organisms does
not violate the second law of thermodynamics
• Entropy (disorder) may decrease in an
organism, but the universe’s total entropy
increases
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Concept 8.2: The free-energy change of a
reaction tells us whether or not the reaction
occurs spontaneously
• Biologists want to know which reactions occur
spontaneously and which require input of
energy
• To do so, they need to determine energy
changes that occur in chemical reactions
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Free-Energy Change, ∆∆∆∆G
• A living system’s free energy is energy that
can do work when temperature and pressure
are uniform, as in a living cell
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• The change in free energy (∆G) during a
process is related to the change in enthalpy, or
change in total energy (∆H), change in entropy
(∆S), and temperature in Kelvin (T)
∆G = ∆H – T∆S
• Only processes with a negative ∆G are
spontaneous
• Spontaneous processes can be harnessed to
perform work
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Free Energy, Stability, and Equilibrium
• Free energy is a measure of a system’s
instability, its tendency to change to a more
stable state
• During a spontaneous change, free energy
decreases and the stability of a system
increases
• Equilibrium is a state of maximum stability
• A process is spontaneous and can perform
work only when it is moving toward equilibrium
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Figure 8.5
• More free energy (higher G) • Less stable • Greater work capacity
In a spontaneous change • The free energy of the system decreases (∆∆∆∆G <<<< 0) • The system becomes more stable • The released free energy can be harnessed to do work
• Less free energy (lower G) • More stable • Less work capacity
(a) Gravitational motion (b) Diffusion (c) Chemical reaction
Figure 8.5a
• More free energy (higher G) • Less stable • Greater work capacity
In a spontaneous change • The free energy of the system decreases (∆∆∆∆G <<<< 0) • The system becomes more stable • The released free energy can be harnessed to do work
• Less free energy (lower G) • More stable • Less work capacity
Figure 8.5b
(a) Gravitational motion (b) Diffusion (c) Chemical reaction
Free Energy and Metabolism
• The concept of free energy can be applied to
the chemistry of life’s processes
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Exergonic and Endergonic Reactions in
Metabolism
• An exergonic reaction proceeds with a net
release of free energy and is spontaneous
• An endergonic reaction absorbs free energy
from its surroundings and is nonspontaneous
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Figure 8.6 (a) Exergonic reaction: energy released, spontaneous
(b) Endergonic reaction: energy required, nonspontaneous
Reactants
Energy
Products
Progress of the reaction
Amount of energy released (∆∆∆∆G <<<< 0)
Reactants
Energy
Products
Amount of energy required (∆∆∆∆G >>>> 0)
Progress of the reaction
Free energy
Free energy
Figure 8.6a
(a) Exergonic reaction: energy released, spontaneous
Reactants
Energy
Products
Progress of the reaction
Amount of energy released (∆∆∆∆G <<<< 0)
Free energy
Figure 8.6b
(b) Endergonic reaction: energy required, nonspontaneous
Reactants
Energy
Products
Amount of energy required (∆∆∆∆G >>>> 0)
Progress of the reaction
Free energy
Equilibrium and Metabolism
• Reactions in a closed system eventually reach
equilibrium and then do no work
• Cells are not in equilibrium; they are open
systems experiencing a constant flow of materials
• A defining feature of life is that metabolism is
never at equilibrium
• A catabolic pathway in a cell releases free energy
in a series of reactions
• Closed and open hydroelectric systems can
serve as analogies
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Figure 8.7
(a) An isolated hydroelectric system
(b) An open hydro- electric system
(c) A multistep open hydroelectric system
∆∆∆∆G <<<< 0
∆∆∆∆G <<<< 0
∆∆∆∆G <<<< 0 ∆∆∆∆G <<<< 0
∆∆∆∆G <<<< 0
∆∆∆∆G ==== 0
Figure 8.7a
(a) An isolated hydroelectric system
∆∆∆∆G <<<< 0 ∆∆∆∆G ==== 0
Figure 8.7b
(b) An open hydroelectric system
∆∆∆∆G <<<< 0
Figure 8.7c
(c) A multistep open hydroelectric system
∆∆∆∆G <<<< 0
∆∆∆∆G <<<< 0
∆∆∆∆G <<<< 0
Concept 8.3: ATP powers cellular work by
coupling exergonic reactions to endergonic
reactions
• A cell does three main kinds of work
– Chemical
– Transport
– Mechanical
• To do work, cells manage energy resources by
energy coupling, the use of an exergonic
process to drive an endergonic one
• Most energy coupling in cells is mediated by ATP
© 2011 Pearson Education, Inc.
The Structure and Hydrolysis of ATP
• ATP (adenosine triphosphate) is the cell’s
energy shuttle
• ATP is composed of ribose (a sugar), adenine
(a nitrogenous base), and three phosphate
groups
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Figure 8.8
(a) The structure of ATP
Phosphate groups
Adenine
Ribose
Adenosine triphosphate (ATP)
Energy
Inorganic phosphate
Adenosine diphosphate (ADP)
(b) The hydrolysis of ATP
Figure 8.8a
(a) The structure of ATP
Phosphate groups
Adenine
Ribose
Figure 8.8b
Adenosine triphosphate (ATP)
Energy
Inorganic phosphate
Adenosine diphosphate (ADP)
(b) The hydrolysis of ATP
• The bonds between the phosphate groups
of ATP’s tail can be broken by hydrolysis
• Energy is released from ATP when the
terminal phosphate bond is broken
• This release of energy comes from the
chemical change to a state of lower free
energy, not from the phosphate bonds
themselves
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How the Hydrolysis of ATP Performs Work
• The three types of cellular work (mechanical,
transport, and chemical) are powered by the
hydrolysis of ATP
• In the cell, the energy from the exergonic
reaction of ATP hydrolysis can be used to
drive an endergonic reaction
• Overall, the coupled reactions are exergonic
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Figure 8.9
Glutamic acid
Ammonia Glutamine
(b) Conversion reaction coupled with ATP hydrolysis
Glutamic acid conversion to glutamine
(a)
(c) Free-energy change for coupled reaction
Glutamic acid
Glutamine Phosphorylated intermediate
Glu
NH3 NH2
Glu ∆∆∆∆GGlu = +3.4 kcal/mol
ATP ADP ADP
NH3
Glu Glu
P P i
P i ADP
Glu
NH2
∆∆∆∆GGlu = +3.4 kcal/mol
Glu Glu
NH3 NH2 ATP
∆∆∆∆GATP = −−−−7.3 kcal/mol ∆∆∆∆GGlu = +3.4 kcal/mol
+ ∆∆∆∆GATP = −−−−7.3 kcal/mol
Net ∆∆∆∆G = −−−−3.9 kcal/mol
1 2
• ATP drives endergonic reactions by
phosphorylation, transferring a phosphate
group to some other molecule, such as a
reactant
• The recipient molecule is now called a
phosphorylated intermediate
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Figure 8.10 Transport protein Solute
ATP
P P i
P i ADP
P i ADP ATP ATP
Solute transported
Vesicle Cytoskeletal track
Motor protein Protein and vesicle moved
(b) Mechanical work: ATP binds noncovalently to motor proteins and then is hydrolyzed.
(a) Transport work: ATP phosphorylates transport proteins.
The Regeneration of ATP
• ATP is a renewable resource that is
regenerated by addition of a phosphate
group to adenosine diphosphate (ADP)
• The energy to phosphorylate ADP comes
from catabolic reactions in the cell
• The ATP cycle is a revolving door through
which energy passes during its transfer from
catabolic to anabolic pathways
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Figure 8.11
Energy from
catabolism (exergonic,
energy-releasing
processes)
Energy for cellular
work (endergonic,
energy-consuming
processes)
ATP
ADP P i
H2O
Concept 8.4: Enzymes speed up metabolic
reactions by lowering energy barriers
• A catalyst is a chemical agent that speeds up
a reaction without being consumed by the
reaction
• An enzyme is a catalytic protein
• Hydrolysis of sucrose by the enzyme sucrase
is an example of an enzyme-catalyzed
reaction
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Figure 8.UN02
Sucrase
Sucrose
(C12H22O11)
Glucose
(C6H12O6)
Fructose
(C6H12O6)
The Activation Energy Barrier
• Every chemical reaction between molecules
involves bond breaking and bond forming
• The initial energy needed to start a chemical
reaction is called the free energy of activation,
or activation energy (EA)
• Activation energy is often supplied in the form
of thermal energy that the reactant molecules
absorb from their surroundings
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Figure 8.12
Transition state
Reactants
Products
Progress of the reaction
Free energy
EA
∆∆∆∆G <<<< O
A B
C D
A B
C D
A B
C D
How Enzymes Lower the EA Barrier
• Enzymes catalyze reactions by lowering the EA
barrier
• Enzymes do not affect the change in free
energy (∆G); instead, they hasten reactions
that would occur eventually
© 2011 Pearson Education, Inc.
Animation: How Enzymes Work
Figure 8.13
Course of reaction without enzyme
EA
without
enzyme EA with enzyme is lower
Course of reaction with enzyme
Reactants
Products
∆∆∆∆G is unaffected by enzyme
Progress of the reaction
Free energy
Substrate Specificity of Enzymes
• The reactant that an enzyme acts on is called the
enzyme’s substrate
• The enzyme binds to its substrate, forming an
enzyme-substrate complex
• The active site is the region on the enzyme
where the substrate binds
• Induced fit of a substrate brings chemical
groups of the active site into positions that
enhance their ability to catalyze the reaction
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Figure 8.14
Substrate
Active site
Enzyme Enzyme-substrate complex
(a) (b)
Catalysis in the Enzyme’s Active Site
• In an enzymatic reaction, the substrate binds to
the active site of the enzyme
• The active site can lower an EA barrier by
– Orienting substrates correctly
– Straining substrate bonds
– Providing a favorable microenvironment
– Covalently bonding to the substrate
© 2011 Pearson Education, Inc.
Figure 8.15-1
Substrates
Substrates enter active site.
Enzyme-substrate complex
Substrates are held in active site by weak interactions.
1 2
Enzyme
Active site
Figure 8.15-2
Substrates
Substrates enter active site.
Enzyme-substrate complex
Substrates are held in active site by weak interactions.
Active site can lower EA and speed up a reaction.
1 2
3
Substrates are converted to products.
4
Enzyme
Active site
Figure 8.15-3
Substrates
Substrates enter active site.
Enzyme-substrate complex
Enzyme
Products
Substrates are held in active site by weak interactions.
Active site can lower EA and speed up a reaction.
Active site is
available for two new substrate molecules.
Products are released.
Substrates are converted to products.
1 2
3
4 5
6
Effects of Local Conditions on Enzyme
Activity
• An enzyme’s activity can be affected by
– General environmental factors, such as
temperature and pH
– Chemicals that specifically influence the
enzyme
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Effects of Temperature and pH
• Each enzyme has an optimal temperature in
which it can function
• Each enzyme has an optimal pH in which it can
function
• Optimal conditions favor the most active shape
for the enzyme molecule
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Figure 8.16
Optimal temperature for typical human enzyme (37°°°°C)
Optimal temperature for
enzyme of thermophilic
(heat-tolerant)
bacteria (77°°°°C)
Temperature (°°°°C)
(a) Optimal temperature for two enzymes
Rate of reaction
Rate of reaction
120 100 80 60 40 20 0
0 1 2 3 4 5 6 7 8 9 10 pH
(b) Optimal pH for two enzymes
Optimal pH for pepsin (stomach enzyme)
Optimal pH for trypsin (intestinal enzyme)
Figure 8.16a
Optimal temperature for typical human enzyme (37°°°°C)
Optimal temperature for enzyme of thermophilic
(heat-tolerant) bacteria (77°°°°C)
Temperature (°°°°C)
(a) Optimal temperature for two enzymes
Rate of reaction
120 100 80 60 40 20 0
Figure 8.16b
Rate of reaction
0 1 2 3 4 5 6 7 8 9 10 pH
(b) Optimal pH for two enzymes
Optimal pH for pepsin (stomach enzyme)
Optimal pH for trypsin (intestinal enzyme)
Cofactors
• Cofactors are nonprotein enzyme helpers
• Cofactors may be inorganic (such as a metal in
ionic form) or organic
• An organic cofactor is called a coenzyme
• Coenzymes include vitamins
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Enzyme Inhibitors
• Competitive inhibitors bind to the active site
of an enzyme, competing with the substrate
• Noncompetitive inhibitors bind to another
part of an enzyme, causing the enzyme to
change shape and making the active site less
effective
• Examples of inhibitors include toxins, poisons,
pesticides, and antibiotics
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Figure 8.17
(a) Normal binding (b) Competitive inhibition (c) Noncompetitive inhibition
Substrate
Active site
Enzyme
Competitive inhibitor
Noncompetitive inhibitor
The Evolution of Enzymes
• Enzymes are proteins encoded by genes
• Changes (mutations) in genes lead to changes
in amino acid composition of an enzyme
• Altered amino acids in enzymes may alter their
substrate specificity
• Under new environmental conditions a novel
form of an enzyme might be favored
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Figure 8.18
Two changed amino acids were found near the active site.
Active site
Two changed amino acids were found in the active site.
Two changed amino acids were found on the surface.
Concept 8.5: Regulation of enzyme activity
helps control metabolism
• Chemical chaos would result if a cell’s
metabolic pathways were not tightly regulated
• A cell does this by switching on or off the
genes that encode specific enzymes or by
regulating the activity of enzymes
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Allosteric Regulation of Enzymes
• Allosteric regulation may either inhibit or
stimulate an enzyme’s activity
• Allosteric regulation occurs when a regulatory
molecule binds to a protein at one site and
affects the protein’s function at another site
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Allosteric Activation and Inhibition
• Most allosterically regulated enzymes are
made from polypeptide subunits
• Each enzyme has active and inactive forms
• The binding of an activator stabilizes the
active form of the enzyme
• The binding of an inhibitor stabilizes the
inactive form of the enzyme
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Figure 8.19
Regulatory site (one of four)
(a) Allosteric activators and inhibitors
Allosteric enzyme with four subunits
Active site (one of four)
Active form
Activator
Stabilized active form
Oscillation
Non- functional active site
Inactive form Inhibitor
Stabilized inactive form
Inactive form
Substrate
Stabilized active form
(b) Cooperativity: another type of allosteric activation
Figure 8.19a
Regulatory site (one of four)
(a) Allosteric activators and inhibitors
Allosteric enzyme with four subunits
Active site (one of four)
Active form
Activator
Stabilized active form
Oscillation
Nonfunctional active site
Inactive form Inhibitor
Stabilized inactive form
Figure 8.19b
Inactive form
Substrate
Stabilized active form
(b) Cooperativity: another type of allosteric activation
• Cooperativity is a form of allosteric regulation
that can amplify enzyme activity
• One substrate molecule primes an enzyme to
act on additional substrate molecules more
readily
• Cooperativity is allosteric because binding by a
substrate to one active site affects catalysis in
a different active site
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Identification of Allosteric Regulators
• Allosteric regulators are attractive drug
candidates for enzyme regulation because of
their specificity
• Inhibition of proteolytic enzymes called
caspases may help management of
inappropriate inflammatory responses
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Figure 8.20
Caspase 1 Active site
Substrate
SH SH
SH
Known active form Active form can bind substrate
Allosteric binding site
Allosteric inhibitor
Hypothesis: allosteric inhibitor locks enzyme in inactive form
Caspase 1
Active form Allosterically inhibited form
Inhibitor
Inactive form
EXPERIMENT
RESULTS
Known inactive form
Figure 8.20a
Caspase 1 Active site
Substrate
SH SH
SH
Known active form Active form can
bind substrate
Allosteric
binding site Allosteric
inhibitor Hypothesis: allosteric
inhibitor locks enzyme
in inactive form
EXPERIMENT
Known inactive form
Figure 8.20b
Caspase 1
Active form Allosterically
inhibited form
Inhibitor
Inactive form
RESULTS
Feedback Inhibition
• In feedback inhibition, the end product of a
metabolic pathway shuts down the pathway
• Feedback inhibition prevents a cell from
wasting chemical resources by synthesizing
more product than is needed
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Figure 8.21
Active site available
Isoleucine used up by
cell
Feedback inhibition
Active site of enzyme 1 is
no longer able
to catalyze the
conversion
of threonine to intermediate A;
pathway is
switched off. Isoleucine binds to
allosteric
site.
Initial substrate
(threonine)
Threonine in active site
Enzyme 1 (threonine
deaminase)
Intermediate A
Intermediate B
Intermediate C
Intermediate D
Enzyme 2
Enzyme 3
Enzyme 4
Enzyme 5
End product (isoleucine)
Specific Localization of Enzymes Within
the Cell
• Structures within the cell help bring order to
metabolic pathways
• Some enzymes act as structural components
of membranes
• In eukaryotic cells, some enzymes reside in
specific organelles; for example, enzymes for
cellular respiration are located in mitochondria
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Figure 8.22
Mitochondria
The matrix contains enzymes in solution that are involved in one stage
of cellular respiration.
Enzymes for another stage of cellular respiration are
embedded in the inner membrane.
1 µµµµm
Figure 8.22a
1 µµµµm
Figure 8.UN03
Course of reaction without enzyme
EA without enzyme EA with
enzyme is lower
Course of reaction with enzyme
Reactants
Products
∆∆∆∆G is unaffected by enzyme
Progress of the reaction
Free energy
Figure 8.UN04
Figure 8.UN05
Figure 8.UN06
Figure 8.UN07